Solutions practice · Mixed difficulty

For negative deviation from Raoult’s law, which of the following is an incorrect relation?

Scuba divers may experience a condition called To avoids this, the tanks used by scuba divers are filled with air diluted with

A solution that obeys Raoult’s law is called

If vapour pressure of two liquids A and B in pure state are 400 and 500 mm of Hg respectively then mole fraction of A in vapour phase of solution obtained by mixing equal moles of A and B is

Consider the following statements about osmotic pressure method of molar mass determination.

I. Molarity of the solution is used instead of molality.

II. Magnitude of osmotic pressure is very large even for dilute solutions.

III. Molar mass of biomolecules can be determined as they are not stable at higher temperatures.

IV. Determine the molar mass of polymer as they have poor solubility.

Which of the above statements are responsible for advantage of osmotic pressure for determination of molar mass over the other colligative properties?

The vapour density of undecomposed ${\mathrm{N}_2}{\mathrm{O}_4}$ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to $\mathrm{N}{\mathrm{O}_2}.$ The per cent dissociation of ${\mathrm{N}_2}{\mathrm{O}_4}$ at the final temperature is :

Which has the highest freezing point at one atmosphere?

$\Delta T_f / K_f$ has the same value of $1 \mathrm{~mol} \mathrm{~kg}^{-1}$ for $8 \%$ $A B_2$ and $10 \% A_2 B$ by mass of solvent, both $A B_2$ and $A_2 B$ being non- electrolytes. Atomic masses of $A$ and $B$ will be respectively

The vapour pressure of a liquid in a closed container depends upon

At temperature $327^\circ C$ and concentration C osmotic pressure of a solution is p, the same solutions at concentration C/2 and a temperature $427^\circ C$ shows osmotic pressure 2 atm, value of p will be

When a substance is distributed between two immiscible solvents and remains in the same state in the solvent I, while, dissociates in the solvent II. If the concentration of solute are ${c_\mathrm{I}}\;\mathrm{and}\;{c_{\mathrm{II}}}$ in phase I and II respectively then :

Lowering in vapour pressure is the highest for:

Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A): At $10^\circ C,$ the density of a 5 M solution of $KCl$ [atomic masses of $K\,\,\& \,\,Cl$ are 39 & 35.5 $g\,\,mo{l^{ - 1}}$ respectively] is $'x'\,\,g\,\,m{l^{ - 1}}.$ The solution is cooled to $- 21^\circ C.$ The molality of the solution will remain unchanged.
Reason (R) : The molality of a solution does not change with temperature as mass remains unaffected with temperature.
In the light of the above statements, choose the correct answer from the options given below.

In which ratio of volume $0.4\mathrm{ }\;M\;\mathrm{ }HCl\;\mathrm{ }and\;\mathrm{ }0.9\;\mathrm{ }M\;\mathrm{ }HCl$ are to be mixed such that the concentration of the resultant solution becomes 0.7 M ?

Assertion (A): Sum of mole fraction of all components in a mixture is 1.

Reason (R): Mole fraction is temperature dependent mode of concentration.

The values of observed and calculated molecular weights of silver nitrate are 92.64 and 170 respectively. The degree of dissociation of silver nitrate is :

Which of the following statements is not correct about homogeneous mixtures?

In two solutions having different osmotic pressure, the solution of higher osmotic pressure is called :

Which one of the following aqueous solutions will exhibit highest boiling point?

A and B ideal gases. The molecular weights of A and B are in the ratio of 1:4. The pressure of a gas mixture containing equal weight of A and B is p atm. What is the partial pressure (in atm) of B in the mixture?

The temperature at which vapour pressure of a solvent in its liquid and solid phase becomes same is called :

The vapour pressure of the solution of two liquids $A\left(P^{\circ}=80 \mathrm{mm}\right)$, and $B\left(P^{\circ}=120 \mathrm{mm}\right)$ is found to be $100 \mathrm{mm}$ when $X_{A}=0.4$. The result shows that

If the various terms in the below given expressions have usual meanings, the van’t Hoff factor (i) cannot be calculated by which one of the expressions?

The molal elevation constant for water is $\mathrm{0}\mathrm{.52}\;\mathrm{K}\;\mathrm{molalit}{\mathrm{y}^{ - 1}}$. The elevation caused in the boiling point of water by dissolving 0.25 mole of a non-volatile solute in 250 g of water will be :

The solubility of a gas in water depends on :

On mixing $10 \mathrm{~mL}$ of acetone with $40 \mathrm{~mL}$ of chloroform, the total volume of the solution is :

A solution of protein (extracted from crabs) was prepared by dissolving 0.75 g in $125\;\mathrm{c}{\mathrm{m}^3}$ of an aqueous solution. At $4^\circ C$ an osmotic pressure rise of 2.6 mm of the solution was observed. Then molecular weight of protein is : (Assume density of solution is $1.00\;g/\mathrm{c}{\mathrm{m}^3}$)

Molarity and molality of a solution of ${NaOH}$ is calculated. If now temperature of the solution is increased then which of the following statement(s) is/are correct ?

(i) Molarity of solution decreases

(ii) Molality of the solution increases

Consider the following aqueous solutions and assume 100% ionisation in electrolytes

I. 0.1 m urea

II. 0.04 m $\mathrm{A}{\mathrm{l}_2}{\left( {\mathrm{S}{\mathrm{O}_4}} \right)_3}$

III. 0.05 m $\mathrm{CaC}{\mathrm{l}_2}$

IV. 0.005 m NaCl

The correct statement regarding the above solution is

Which of the following solutions has the highest normality?